20B Section Review 1- How can you tell the difference between solutes.docx
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20B Section Review 1. How can you tell the difference between solutes and solve nts in a solution when they are in the same state? 2. What are the properties of solutions? Which of these are shared with some heterogeneous mixtures? 3. What gas solutions are not possible? Why? 4. Why is water such an effective solvent? 5. Describe the three steps in the solution process. 6. How is dissociation different from ionization? 7. What kinds of substances does the term miscible refer to? What is true about the possible proportions of completely miscible 8. How does the pressure of a gas above a solvent affect the amount 9. How can an unsaturated solution become supersaturated with- 10. Which parts of the solution process are enhanced by stirig 11. (True or False) Solutions differ from most colloidal disersiols substances in solutions? of gas that dissolves in the solvent? What is this principle called? out any solute being added or any by heating? by crushing or grinding? in that their solute particles are uniformly dispersed. solvent being removed? Solution 1.One substance which is dissolved in another substance. Solvent is the one which dissolves the solute. When both are same state form homogeneous mixture of solution with different colour from it\'s individual. 2. Solutions are composition of 2 or more substances in liquid form. Heterogeneous solution is one which has different phases or parts dissolved in solution with different ratio. Visibly different colour or phase. 3. Here solvent is gas. Only gas solute only dissolve in this gas condition not solution(liquid form). So gas solution not possible. 4. Water is the one which has capable of dissolve variety of solute. It it polar in nature. Hydrogen has positive charge and oxygen gas negative charge for polarization. .
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Scientifically continuous phase apersed phase Speaking Chapter Review.docx
Scientifically continuous phase apersed phase Speaking Chapter Review or hono- 458 I. How is a mixture determined to be hetere ty What are the phases of matter that form gelst sols? How ndal effect gels and sols different? 3. What property of the liquids in an emulsion would work against their forming any kind of mixture?em to 4. How can you tell that a rock is a heterogeneous clation inty \'s law 5. What property do colloidal dispersions and solutions that other kinds of mixtures do not? is a col. 470 472 472 473 6. What is one property of skim milk indicating that it 31 loidal dispersion? tage by mass ve properties -point depression oint elevation 7. How might you visually tell the difference between a sion and a colloidal dispersion? 474 8. What can happen when metals with very different-sized are mixed in heterogeneous alloys? 9. Which part of a solution is the solvent? How is this inf used to classify the solution? 10. When you mix a solid and a liquid, what are two indication that a solution was formed and not a new compound? 11. What are solutions of different metals called? Why are often preferred to pure metals? 12. Why is it not possible to have a solid-in-gas solution? 13. Why is the water molecule electrically polar? 14. Why is solvation of a solute particle an important step in d 15. What kind of solvent could dissolve a nonpolar solute like sul. 16. Explain the difference between the terms soluble and solubility 18. How can you tell when a solid-in-liquid solution is saturated? solving the solute? What do we call the solution ionic solutes? process for fur? Explain your answer Explain why the solubility of gases normally decreases with ris ing temperature. 17. 19. Where does the solution process take place on a piece of a solid solute? How can you increase the rate of solution in light of this fact? 20. What instrument could be used to measure a mole of solid sol- ute particles? Why can this instrument be used? 21. Which solution would have a lower boiling point, one with 1.0 mol of solute particles or one with 2.0 mol? Explain. DS 0 22. Some conservationists are disturbed by the large amount of brine that is pumped back into the ocean by desalination plants. Why could it be a problem? What could be done to re- duce the effects of returning concentrated brine to the sea?
Solution
in case of multiple questions being posted i am allowed to answer the first question. please post one question at one time.
Answer 1)
A homogeneous mixture has the same appearence and compostion throughout. wheras a heterogenous mixture would consist of visibly different phases or substances like solid-liquid or suspensions
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Scientifically continuous phase apersed phase Speaking Chapter Review.docx
Scientifically continuous phase apersed phase Speaking Chapter Review or hono- 458 I. How is a mixture determined to be hetere ty What are the phases of matter that form gelst sols? How ndal effect gels and sols different? 3. What property of the liquids in an emulsion would work against their forming any kind of mixture?em to 4. How can you tell that a rock is a heterogeneous clation inty \'s law 5. What property do colloidal dispersions and solutions that other kinds of mixtures do not? is a col. 470 472 472 473 6. What is one property of skim milk indicating that it 31 loidal dispersion? tage by mass ve properties -point depression oint elevation 7. How might you visually tell the difference between a sion and a colloidal dispersion? 474 8. What can happen when metals with very different-sized are mixed in heterogeneous alloys? 9. Which part of a solution is the solvent? How is this inf used to classify the solution? 10. When you mix a solid and a liquid, what are two indication that a solution was formed and not a new compound? 11. What are solutions of different metals called? Why are often preferred to pure metals? 12. Why is it not possible to have a solid-in-gas solution? 13. Why is the water molecule electrically polar? 14. Why is solvation of a solute particle an important step in d 15. What kind of solvent could dissolve a nonpolar solute like sul. 16. Explain the difference between the terms soluble and solubility 18. How can you tell when a solid-in-liquid solution is saturated? solving the solute? What do we call the solution ionic solutes? process for fur? Explain your answer Explain why the solubility of gases normally decreases with ris ing temperature. 17. 19. Where does the solution process take place on a piece of a solid solute? How can you increase the rate of solution in light of this fact? 20. What instrument could be used to measure a mole of solid sol- ute particles? Why can this instrument be used? 21. Which solution would have a lower boiling point, one with 1.0 mol of solute particles or one with 2.0 mol? Explain. DS 0 22. Some conservationists are disturbed by the large amount of brine that is pumped back into the ocean by desalination plants. Why could it be a problem? What could be done to re- duce the effects of returning concentrated brine to the sea?
Solution
in case of multiple questions being posted i am allowed to answer the first question. please post one question at one time.
Answer 1)
A homogeneous mixture has the same appearence and compostion throughout. wheras a heterogenous mixture would consist of visibly different phases or substances like solid-liquid or suspensions
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Solution
After studying chapter 7 learning objectives, you should be able to:
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Protection:
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Solution
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In c,
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In c,
Topic pointers
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Topic pointers
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Solution
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XÂ Â Â x;
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Solution
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Answer -
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Solution
true
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Solution
H ello Pal,
F irst of all a very nice as well as intersting question from your side.
S o now straight to the question, as asked above with all the information available from your side and from mine, the answer is as under:
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Solution
Advantages
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Solution
Answer
From following the agents likely cause security related problems to the AIS.
From Employees
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Generally provides the Security Service management Supplier, they provide both security services and management thereof.
Security management service will be conducted by Service Supplier.
.
Im creating a stack class using generics- what should my peek method l.docx
Im creating a stack class using generics. what should my peek method look like ? I\'m just using a simple peek method, here\'s what i have thus far
public class stack<T>
{
private ArrayList<T> stack = new ArrayList<T> ();
private int top = 0;
public int size () {
return top;
}
public void push (T item) {
stack.add (top++, item);
}
public T pop () {
return stack.remove (--top);
}
public T peek()
{
}
public Boolean isEmpty()
{
if (top == -1)
return true;
else
return false;
}
}
Solution
Hi,
I have updated peek() methd. Highlighted code changes.
public class stack<T>
{
private ArrayList<T> stack = new ArrayList<T> ();
private int top = 0;
public int size () {
return top;
}
public void push (T item) {
stack.add (top++, item);
}
public T pop () {
return stack.remove (--top);
}
public T peek()
{
if (isEmpty()) {
throw new EmptyStackException();
}
return stack.get(top);
}
public Boolean isEmpty()
{
if (top == -1)
return true;
else
return false;
}
}
.
ii)State whether you would expect the following Group 13 metal cations.docx
ii)State whether you would expect the following Group 13 metal cations to act as Lewis acids or bases. Order the cations in terms of softest to hardest. Explain your answer. Al3+, Tl3+, Ga3+, Tl+
(iii) State whether you would expect the following Group 15 hydrides to act as Lewis acids or bases. Order the hydrides in terms of softest to hardest. Explain your answer. PH3, NH3, AsH3
Solution
ii) The given group 13 metal cations will act as a Lewis acids , because cations are are electron deficient and act as a electron acceptor.
Hard Acids are Lewis acid which are small in size and most likely are the light metal cation with high positive oxidation state like Al 3+
Soft Acids are Lewis acid which are larger in size and most likely are the heavy metal cation associated with low oxidation state like Tl 3+ Tl +
Oder of cation from softest to hardest   Tl + < Tl 3+ < Al 3+
(iii) The given Group 15 hydrides will acts as Lewis Base, because Nitrogen, Phosphorus and Arsenic has a lone pair of electron that it can donate.
Hard Base are Lewis base anions or neutral molecules which are not easily polarizable like NH 3
Soft Base are Lewis base anions or neutral molecules which are easily polarizable like PH 3 and AsH 3
Order the hydrides in terms of softest to hardest AsH 3 < PH 3 <NH 3
.
IMF in Greece- Good or bad for the country- Why-SolutionIMF is interna.docx
IMF in Greece. Good or bad for the country? Why?
Solution
IMF is international monetary fund.It was established with the motive of promoting international monetary cooperation.It is good because:
1. It helps in abolishing the exchange restrictions among member nations.
2. It helps in maintaining balanced economic development of the member nations by poviding them monetary help.
3. It helps the member countries in making investment in profitable projects.
4. It offers monetary help to member countries in correcting the disequilibrium of balance of payment.
IMF is bad because:
1. it is a club of rich countries only. it discriminate between rich and poor memebers.
2. it do not provides loan for developmental projects. it only gives loans for maintaining the favourable balance of payment.
3. it interferes in the domestic economies of member countries. while providing loan to member counties IMF put many restrictions.
4. IMF tried to maintain stability in price of gold but failed in achieving this aim.
.
2- What is a colloid- Why is it difficult to filter a colloid- 3- What.docx
2. What is a colloid? Why is it difficult to filter a colloid? 3. What is coagulation? What is peptization? 4. Why is the solution of AgNOs added slowly? 5. Why must a large excess of AgNOs be avoided? 6. Why must the silver chloride be protected from the light? 7. For simplicity assume that your unknown chloride is NaCl. Calculate how many mL of the 5% AgNO3 solution must be added to 0.4020 g of the NaCl sample to precipitate all the chloride. Note: 5% means that there are 5 grams of silver nitrate per 100 mL of solution.
Solution
2) Colloid : Colloid is a dispersion of small tiny particles in a liquid.. In collods the tiny particles remain suspended in the solvent. rather than settling at the bottom.
It is difficult to filter collodal solution because these tiny particles pass through the filter paper.
3) Coagulation : means the aggrigation of oppositely charged particles which settle down under the gravity.
Peptization : It is a phenomenon of the formation of a colloidal dispersion from precipitation.
4)Addition of the AgNO3 be done slowly because the addition tends to yield large particles which makes filtration more efficiently .It also helps limit coprecipitation.
5)To avoid coprecipatation the excess of AgNO3 be avoided.
6)Silver chloride must be protected from light as it is unstable. Exposure to light it becomes greyish yellow . Hence, to avoid decompostion, it must be protected from light.
.
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